Homework Answers
When you add water to unknown acid strength of acetic acid, pH at half equivalence point will be equal to pKa of the acid will remain same.
pKa is independent of concentration.
The volume of NaOH needed to reach equivalence will remain same as the total number of moles of acetic acid in the flask remains same.
The concentration of acetate ions at equivalence point will also remain same as that of previous titration.
pH at the start of the titration will increase. This is because , dilution decreases H+ concentration. Thus, pH will be higher.
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Question 6 (1 point) In your pre-lab, you were asked to determine the concentration for a...
Question 6 (1 point) In your pre-lab, you were asked to determine the concentration for a...
Question 6 (1 point) In your pre-lab, you were asked to determine the concentration for a 25.00 mL sample of acetic acid, CH3COOH (K= 1.8 x 10-5) of unknown concentration. Suppose you now repeat that same titration, using another 25.00 mL sample of that same unknown acetic acid and the same concentration of NaOH as a titrant. However, before you start titrating, you add an additional 100 mL of water to the flask containing our sample of acid. Everything else...
Which of the statements below is/are true of your solution at equivalence? Select all true statements...
Which of the statements below is/are true of your solution at equivalence? Select all true statements below. The concentration of acetate ions (CH2C00) at equivalence is the same as the original concentration of acetic acid (CH2COOH) at the start of the titration (i.e. 1.0 M). The number of moles of acetate ions (CH3COO") at equivalence is the same as the number of moles of of acetic acid (CH2COOH) at the start of the titration (i.e. 0.10 mol). At the equivalence...
In your pre-lab, we asked you to consider a few of the properties you could measure...
In your pre-lab, we asked you to consider a few of the properties you could measure during the titration of a 100.0 mL sample of 1.0 M acetic acid, CH3COOH (Ka = 1.8 x 10-5) with 0.50 mol/L NaOH solution at 25°C. Let's think about this same titration again, this time at the molecular-scale. Question 2 (1 point) After you have added a total of 100.0 mL of NaOH (aq), what are the major species in your beaker other than...
please help with my pre lab additional information Pre-Lab Questions: 1. What is the definition of...
please help with my pre lab
additional information
Pre-Lab Questions: 1. What is the definition of an 'equivalence point' in an acid/base titration? (1 point) 2. In part one of the experiment, you will prepare the acid solutions being titrated from a stock solution. Describe how you will accurately prepare 10.00 mL of 0.100 M HCl solution using a 1.00 M HCI stock solution. In your response to this question, be very specific about the quantities of stock solution and...
Pre-Lab Questions The titration curve below (on the next page) was obtained by titrating 25.00 mL...
i need help with pre-lab questions
Pre-Lab Questions The titration curve below (on the next page) was obtained by titrating 25.00 mL of a boric acid solution with a 1.000 M NaOH solution. Use the information given on the titration curve to answer the following questions: 1. What is the formula and value of K, for boric acid? Calculate using the half equivalence data point, and using the pH at one-quarter and three-quarter points, too. What is the average Ka...
If you could please help me with these that would be amazing! Thanks in advance Pre-Lab...
If you could please help me with these that would be
amazing! Thanks in advance
Pre-Lab Assignment for Experiment 19:Titration Curves Introduction: This pre-lab assignment will illustrate some of the important features of titration curves and what information can be obtained from them. A titration curve is the plot of the pH of a solution such as an acid or a base as a titrant is being added to it. A titrant is the solution being added from a buret,...
40.0 ml of an acetic acid of unknown concentration is titrated with 0.100 M NaOH. After...
40.0 ml of an acetic acid of unknown concentration is titrated with 0.100 M NaOH. After 20.0 mL of the base solution has been added, the pH in the titration flask is 5.10. What was the concentration of the original acetic acid solution? [Ka(CH3COOH) = 1.8 × 10–5]
In the second image it states that after I pass the equivalence point, I should add...
In the second image it states that after I
pass the equivalence point, I should add 2ml of aliquots of NaOH
until there's no PH change. How do I identify when the equivalence
point is?
Preparation of the unknown weak acid Select the NaOH and fill the buret with the now standardized NaOH solution. [NaOH]=0.097M Record the initial buret volume in your Notebook. 3 Using the volumetric pipet, transfer 25.00 mL of the unknown weak acid to the Erlenmeyer flask....
1. What is the definition of an 'equivalence point' in an acid/base titration? (1 point) 2....
1. What is the definition of an 'equivalence point' in an acid/base titration? (1 point) 2. In part one of the experiment, you will prepare the acid solutions being titrated from a stock solution. Describe how you will accurately prepare 10.00 mL of 0.100 M HCl solution using a 1.00 M HCl stock solution. In your response to this question, be very specific about the quantities of stock solution and deionized water to be used in the dilution and the...
Titration of weak acid with strong base pre-lab Answers can only be entered/graded between 2019-10-24 and...
Titration of weak acid with strong base pre-lab
Answers can only be entered/graded between 2019-10-24 and 2019-10-29 A student peforms a titration, titrating 25.00 mL of a weak monoprotic acid, HA, with a 1.12 M solution of NaOH. They collect data, plot a titration curve and determine the values given in the below table. ml NaOH PH added Half-way Point 17.97 3.66 Equivalence point 35.938.65 How many moles of NaOH have been added at the equivalence point? r mol correct...
Question 6 (1 point) In your pre-lab, you were asked to determine the concentration for a 25.00 mL sample of acetic acid, CH3COOH (K= 1.8 x 10-5) of unknown concentration. Suppose you now repeat that same titration, using another 25.00 mL sample of that same unknown acetic acid and the same concentration of NaOH as a titrant. However, before you start titrating, you add an additional 100 mL of water to the flask containing our sample of acid. Everything else...
Which of the statements below is/are true of your solution at equivalence? Select all true statements below. The concentration of acetate ions (CH2C00) at equivalence is the same as the original concentration of acetic acid (CH2COOH) at the start of the titration (i.e. 1.0 M). The number of moles of acetate ions (CH3COO") at equivalence is the same as the number of moles of of acetic acid (CH2COOH) at the start of the titration (i.e. 0.10 mol). At the equivalence...
In your pre-lab, we asked you to consider a few of the properties you could measure during the titration of a 100.0 mL sample of 1.0 M acetic acid, CH3COOH (Ka = 1.8 x 10-5) with 0.50 mol/L NaOH solution at 25°C. Let's think about this same titration again, this time at the molecular-scale. Question 2 (1 point) After you have added a total of 100.0 mL of NaOH (aq), what are the major species in your beaker other than...
please help with my pre lab
additional information
Pre-Lab Questions: 1. What is the definition of an 'equivalence point' in an acid/base titration? (1 point) 2. In part one of the experiment, you will prepare the acid solutions being titrated from a stock solution. Describe how you will accurately prepare 10.00 mL of 0.100 M HCl solution using a 1.00 M HCI stock solution. In your response to this question, be very specific about the quantities of stock solution and...
i need help with pre-lab questions
Pre-Lab Questions The titration curve below (on the next page) was obtained by titrating 25.00 mL of a boric acid solution with a 1.000 M NaOH solution. Use the information given on the titration curve to answer the following questions: 1. What is the formula and value of K, for boric acid? Calculate using the half equivalence data point, and using the pH at one-quarter and three-quarter points, too. What is the average Ka...
If you could please help me with these that would be
amazing! Thanks in advance
Pre-Lab Assignment for Experiment 19:Titration Curves Introduction: This pre-lab assignment will illustrate some of the important features of titration curves and what information can be obtained from them. A titration curve is the plot of the pH of a solution such as an acid or a base as a titrant is being added to it. A titrant is the solution being added from a buret,...
In the second image it states that after I
pass the equivalence point, I should add 2ml of aliquots of NaOH
until there's no PH change. How do I identify when the equivalence
point is?
Preparation of the unknown weak acid Select the NaOH and fill the buret with the now standardized NaOH solution. [NaOH]=0.097M Record the initial buret volume in your Notebook. 3 Using the volumetric pipet, transfer 25.00 mL of the unknown weak acid to the Erlenmeyer flask....
1. What is the definition of an 'equivalence point' in an acid/base titration? (1 point) 2. In part one of the experiment, you will prepare the acid solutions being titrated from a stock solution. Describe how you will accurately prepare 10.00 mL of 0.100 M HCl solution using a 1.00 M HCl stock solution. In your response to this question, be very specific about the quantities of stock solution and deionized water to be used in the dilution and the...
Titration of weak acid with strong base pre-lab
Answers can only be entered/graded between 2019-10-24 and 2019-10-29 A student peforms a titration, titrating 25.00 mL of a weak monoprotic acid, HA, with a 1.12 M solution of NaOH. They collect data, plot a titration curve and determine the values given in the below table. ml NaOH PH added Half-way Point 17.97 3.66 Equivalence point 35.938.65 How many moles of NaOH have been added at the equivalence point? r mol correct...
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